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Chapter 10: Q10.35P (page 406)

Determine the electron-group arrangement, molecular shape, and ideal bond angle(s) for each of the following:

(a)SO42-

(b)NO2-

(c)PH3

Short Answer

Expert verified

The shapes and bond angles of molecules can be determined from the VSEPR theory. The deviations arise mainly due to lone pair-lone pair repulsions.

Step by step solution

01

Step 1:  SO42-

The shape of the molecule is Tetrahedral. The central sulphur atom is sp3hybridized with an expected bond angle of109.5o. However, lone pair-bond pair repulsion on sulphur reduces the bond angle from the expected value.

02

Step 2: NO2-

The molecule has a bent or V-shaped shape. The nitrogen atom is sp3hybridized with an expected bond angle of120o.The lone pair on nitrogen reduces the bond angle from the expected value.

03

Step 3: PH3

The shape of the molecule is Pyramidal. The phosphrous atom is sp3hybridized with expected bond angle of109.5o. However, the lone pair on phosphorous reduces the bond angle from the expected value.

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Most popular questions from this chapter

The VSEPR model was developed before any xenon compounds had been prepared. Thus, these compounds provided an excellent test of the model’s predictive power. What would you have predicted for the shapes of XeF2,XeF4,andXeF6?

An experiment requires 50.0 mL of 0.040 M NaOH for the titration of 1.00 mmol of acid. Mass analysis of the acid shows 2.24% hydrogen, 26.7% carbon, and 71.1% oxygen. Draw the Lewis structure of the acid.

Which molecule in each pair has the greater dipole moment?Give the reason for your choice.

  1. ClO2orSO2
  2. HBr or HCl
  3. BeCl2orSCl2
  4. AsF3orAsF5

Determine the shape around each central atom in each molecule, and explain any deviation from ideal bond angles: (a)H2SO3 (no H-S bond) (b) N2O3(ONNO2)

A molecule of formula AY3 is found experimentally to be polar. Which molecular shapes are possible and which are impossible for AY3?

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